Ground Vs Excited Configurations Worksheet Quick Guide

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Ground Vs Excited Configurations Worksheet

When studying the behavior of electrons in atoms, chemists often use the concept of electronic configurations to describe the distribution of electrons within an atom’s energy levels. These configurations provide valuable information about an atom’s reactivity, stability, and bonding properties. Two common types of electronic configurations are ground state and excited state configurations. In this worksheet, we will explore the differences between ground and excited configurations and practice determining the electronic configurations of various atoms.

Ground State Configurations

The ground state electronic configuration of an atom represents the arrangement of electrons in its lowest energy levels. In these configurations, electrons are placed in orbitals according to the aufbau principle, which states that electrons will fill orbitals starting from the lowest energy level and moving to higher energy levels. Ground state configurations are stable and represent the most energetically favorable arrangement of electrons for a given atom.

For example, the ground state electronic configuration of carbon (Z = 6) is 1s2 2s2 2p2. In this configuration, the first two electrons are placed in the 1s orbital, the next two electrons are placed in the 2s orbital, and the final two electrons are placed in the 2p orbital. This arrangement follows the aufbau principle and represents the lowest energy configuration for the carbon atom.

Excited State Configurations

Excited state electronic configurations occur when electrons within an atom are temporarily promoted to higher energy levels. This promotion can occur when atoms absorb energy, such as through the absorption of light or heat. Excited state configurations are less stable than ground state configurations and represent a temporary arrangement of electrons that occurs when atoms are in an energetically unfavorable state.

Using the example of carbon, if an atom were to absorb energy and transition to an excited state, the electronic configuration may change to 1s2 2s1 2p3. In this excited state, one of the electrons from the 2s orbital has been promoted to the 2p orbital, resulting in a different arrangement of electrons than the ground state configuration. Excited state configurations are temporary and atoms will typically return to their ground state configuration once the absorbed energy is released.

Determining Ground Vs Excited Configurations

When determining whether an electronic configuration is in the ground state or an excited state, it is important to consider the energy levels of the orbitals and the number of electrons present. Ground state configurations will follow the aufbau principle and represent the lowest energy arrangement of electrons for a given atom. Excited state configurations occur when electrons are temporarily promoted to higher energy levels and will typically involve electrons being moved to higher orbitals.

To practice determining ground vs. excited configurations, let’s consider the electronic configurations of several atoms:

1. Oxygen (Z = 8)

Ground state configuration: 1s2 2s2 2p4

Excited state configuration: 1s2 2s1 2p5

2. Sodium (Z = 11)

Ground state configuration: 1s2 2s2 2p6 3s1

Excited state configuration: 1s2 2s2 2p6 3s2

3. Neon (Z = 10)

Ground state configuration: 1s2 2s2 2p6

Excited state configuration: N/A (Neon is a noble gas and does not readily form excited state configurations)

By comparing the ground state and excited state configurations of these atoms, we can see how the arrangement of electrons changes when atoms are in different energy states. Ground state configurations represent the lowest energy arrangement of electrons, while excited state configurations involve electrons being promoted to higher energy levels temporarily.

In summary, electronic configurations provide valuable information about an atom’s reactivity, stability, and bonding properties. Ground state configurations represent the lowest energy arrangement of electrons, while excited state configurations occur when electrons are temporarily promoted to higher energy levels. By practicing determining ground vs. excited configurations, we can better understand the behavior of electrons in atoms and how they influence an atom’s properties.

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